A compound that contains only C and H was burned in excess O2 to give CO2 and H2O. When 0.270 g of the com- pound was burned, the amount of CO2 formed reacted completely with 20.0 mL of 2.00 M NaOH solution according to the equation 2 OH-1aq2 + CO21g2 S CO 2- 1aq2 + H2O1l2 When 0.270 g of the compound was dissolved in 50.0 g of camphor, the resulting solution had a freezing point of 177.9 °C. [#Pure camphor freezes at 179.8 °C and has Kf = 37.7 1°C kg2>mol.] (a) What is the empirical formula of the compound?

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Determine the moles of CO2 produced by using the volume and molarity of NaOH. Since the reaction between CO2 and NaOH is a 1:2 ratio, calculate the moles of CO2 based on the stoichiometry of the reaction.

Convert the moles of CO2 to grams using the molar mass of CO2. This gives the mass of carbon in the original compound.

Calculate the mass of hydrogen in the original compound by subtracting the mass of carbon from the total mass of the compound.

Determine the moles of carbon and hydrogen in the compound using their respective molar masses.

Find the simplest whole number ratio of moles of carbon to moles of hydrogen to determine the empirical formula of the compound.

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주요 개념

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Empirical Formula

The empirical formula of a compound represents the simplest whole-number ratio of the elements present in that compound. It is determined by analyzing the composition of the compound, often through combustion analysis, which provides the amounts of carbon and hydrogen produced. This ratio is crucial for understanding the basic structure of the compound and is foundational in stoichiometry.

Combustion Analysis

Combustion analysis is a technique used to determine the elemental composition of organic compounds. In this process, the compound is burned in excess oxygen, producing carbon dioxide and water. The amounts of these products are measured, allowing for the calculation of the moles of carbon and hydrogen in the original compound, which is essential for deriving the empirical formula.

Freezing Point Depression

Freezing point depression is a colligative property that describes the lowering of the freezing point of a solvent when a solute is dissolved in it. The extent of this depression depends on the number of solute particles in the solution and is quantified using the formula ΔTf = Kf * m, where Kf is the freezing point depression constant and m is the molality of the solution. This concept is important for determining the molar mass of the compound, which aids in finding its empirical formula.